prepare 1M 100 ml H2SO4, density 1.84
To prepare 1M (1 molar) 100 ml of H2SO4 (sulfuric acid) solution with a density of 1.84 g/ml, we need to calculate the amount of H2SO4 needed.
First, let's understand the concept of molarity. Molarity (M) is a way to measure the concentration of a solution, defined as the number of moles of solute per liter of solution. In order to calculate the amount of solute, we need to know the molar mass of H2SO4.
The molar mass of H2SO4 is:
2(1.007 g/mol) + 1(32.06 g/mol) + 4(16.00 g/mol) = 98.09 g/mol
Since we want to prepare a 1M solution, this means we need 1 mole of H2SO4 in 1 liter (1000 ml) of solution. To calculate the amount required for 100 ml, we can use the equation:
Moles of solute = Molarity x Volume
Moles of H2SO4 = 1 M x 100 ml/1000 ml = 0.1 moles
Now, we can calculate the mass of H2SO4 needed using the molar mass:
Mass = Moles x Molar mass
Mass = 0.1 moles x 98.09 g/mol = 9.81 grams
Since the density of the solution is given as 1.84 g/ml, we can find the volume of the solution:
Volume of solution = Mass / Density
Volume of solution = 9.81 g / 1.84 g/ml ≈ 5.33 ml
Therefore, to prepare 1M 100 ml H2SO4 solution with a density of 1.84 g/ml, you would need approximately 9.81 grams of H2SO4 dissolved in a total volume of approximately 5.33 ml, with the remainder being water to reach the final volume of 100 ml.